mpare the four acetic acid and methanol conductivity measurements. What do they suggest about the bond that attaches the hydrogen atom to the methanol molecule compared to acetic acid?
Liquid= Conductivity
Methanol:
CH3OH (aq) = 0
0.05 M CH3OH (aq)=0
Acetic Acid:
CH3COOH(I)= 0
0.05 M CH3COOH (aq)=265
The addition of H2O to the CH3COOH shows a relatively large increase in conductivity; hence the terminal H of the CH3COOH is more easily broken away (ionized) than the H of the CH3OH. Can't you see that from the measurements?
To compare the conductivity measurements of acetic acid and methanol, we can analyze the data provided. Conductivity is a measure of a substance's ability to conduct electric current, which depends on the presence of ions in the solution.
Looking at the data, we can observe the following measurements:
Methanol:
- CH3OH (aq) = 0 (concentration not specified)
- 0.05 M CH3OH (aq) = 0
Acetic Acid:
- CH3COOH (I) = 0 (concentration not specified)
- 0.05 M CH3COOH (aq) = 265
From the information given, we can infer that the conductivity of methanol, regardless of concentration, is measured as zero. This implies that methanol does not dissociate into ions in solution, and therefore does not contribute to electric current.
On the other hand, the conductivity measurement for acetic acid (0.05 M CH3COOH (aq)) is recorded as 265. This suggests that acetic acid does dissociate into ions in solution, contributing to electric current.
From these findings, we can deduce that the bond between the hydrogen atom and the methanol molecule is stronger compared to the bond between the hydrogen atom and the acetic acid molecule. The stronger bond in methanol leads to a lower degree of dissociation and hence a lack of conductivity. In contrast, the weaker bond in acetic acid facilitates a higher degree of dissociation, resulting in conductivity.